Question

The minimum energy which two molecules should possess so that their collisions result in a chemical reaction is called_________ energy.

Short answer

Answer: Activation energy

Step-by-step solution

Identify the energy type

When two molecules collide, they must have a minimum amount of energy for a chemical reaction to take place. This energy is called Activation energy. Therefore, the filled-in statement will be: The minimum energy which two molecules should possess so that their collisions result in a chemical reaction is called _Activation_ energy.

Key concepts

Understanding Chemical Reactions

A chemical reaction is essentially a process where substances, known as reactants, transform into different substances called products. This transformation occurs through breaking and forming of chemical bonds. For students, visualizing this process can be quite helpful. Imagine each reactant molecule as a puzzle piece, during a chemical reaction, these pieces are rearranged to create a new picture representing the product.

Every chemical reaction is governed by certain laws of chemistry, the most fundamental being the conservation of mass and energy. This means that in a closed system, matter and energy cannot be created or destroyed, only transformed. Hence, when you write a chemical equation, it's important to balance it to reflect this principle. Students are encouraged to use models or diagrams to help in understanding how atoms are rearranged during reactions.

The Role of Molecular Collisions in Reactions

When we talk about molecular collisions, we refer to the instances when two or more molecules bump into each other. However, not all collisions result in a chemical reaction. For a successful chemical reaction to occur, several conditions must be met. First, the molecules must collide with proper orientation to allow for the right atoms to interact. Second, the collision must happen with enough force - energy - to break the initial bonds and start the reaction.

To enhance comprehension of this concept, it's beneficial to think of it in terms of a lock and key mechanism. Only the correct key (collision orientation) that is inserted with enough force (activation energy) can turn the lock (cause a chemical reaction). Illustrating this principle, animations or simulations might come in handy, helping visualize not only the collision but also the energy exchange.

Energy Requirements in Reactions

For reactions to occur, the concept of activation energy is crucial. It's the minimum energy barrier that must be overcome for reactants to be transformed into products. This energy is necessary to break initial bonds so new ones can be formed. It can be visualized as a hurdle in a track race; the runners (reactants) need enough energy to jump over the hurdle (activation energy) to reach the finish line (form products).

In the classroom, employing metaphors like a spark that ignites a fuel can be very beneficial to explain this concept. The spark represents the activation energy needed to start a combustion reaction. To further grasp this idea, interactive activities involving energy diagrams that show the energy of the reactants, the activation energy peak, and the energy of the products can greatly help. These diagrams are not just visual aids but also essential tools for predicting whether a reaction will release or require energy, known as exothermic and endothermic reactions, respectively.